For the reaction PCl3(g)+Cl2(g)--->PCl5(g) the initial mixture contains 4.20 mol PCl3, 5.73 mol Cl2, and no moles of PCl5. At equilibrium, 1.43 mol of PCl3 remains. How many moles of Cl2 and PCl5 are present at equilibrium? (Be sure to give your answer to two decimal places.)
For the reaction PCl3(g)+Cl2(g)--->PCl5(g) the initial mixture contains 4.20 mol PCl3, 5.73 mol Cl2, and no moles of PCl5. At equilibrium, 1.43 mol of PCl3 remains. How many moles of Cl2 and PCl5 are present at equilibrium? (Be sure to give your answer to two decimal places.)
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.2QE: Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium...
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For the reaction
PCl3(g)+Cl2(g)--->PCl5(g)
the initial mixture contains 4.20 mol PCl3, 5.73 mol Cl2, and no moles of PCl5. At equilibrium, 1.43 mol of PCl3 remains.
PCl3(g)+Cl2(g)--->PCl5(g)
the initial mixture contains 4.20 mol PCl3, 5.73 mol Cl2, and no moles of PCl5. At equilibrium, 1.43 mol of PCl3 remains.
How many moles of Cl2 and PCl5 are present at equilibrium? (Be sure to give your answer to two decimal places.)
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